<p>Unit 4 Question Packet Name …………………KEY……………………… The Periodic Table Period ………….</p><p>SKILLS 1. identifying PROPERTIES OF METALS, 4. identifying PROPERTIES OF ELEMENTS METALLOIDS, & NONMETALS 5. explaining PROPERTIES OF ELEMENTS 2. identifying GROUP PROPERTIES 6. identifying TRENDS IN THE PERIDIOC TABLE 3. classifying elements </p><p>SKILL #1: Identifying PROPERTIES OF - refer to your notes & RB p. 19-25 METALS, METALLOIDS, & NONMETALS 1. Write in the space, “metals”, “metalloids”, or “nonmetals” to indicate which type of element each statement is describing. a. metals Located on the left side of the P.T. b. nonmetals Located on the right side of the P.T. c. nonmetals Solids are brittle d. metals Majority of the elements e. nonmetals Gain electrons to form negative ions metalloids Located along the “staircase” g. metals Have luster h. metals Malleable metals Lose electrons to form positive ions metals Ductile k. metals Excellent conductors of heat & electricity nonmetals Poor electrical & heat conductors m. metals Low electronegativity values n. metals Low ionization energy o. nonmetals High ionization energy p. nonmetals High electronegativity values q. nonmetals Ions are larger than their atoms r. metals Ions are smaller than their atoms SKILL #2: Identifying GROUP PROPERTIES - refer to your notes & RB p. 19-25</p><p>2. Write in the space, “Group 1 metals”, “Group 2 metals”, “transition metals”, “halogens”, or “noble gases” to indicate which group each statement is describing. a. Transition metals Colored solutions b. Noble gases Full valence shell c. Group 1 metals Most active metals d. Halogens Most active nonmetals e. Noble gases Monatomic gases Halogens Diatomic elements g. Noble gases Stable and unreactive h. Halogens 7 valence electrons Group 2 metals 2 valence electrons Group 1 metals Form ions with a +1 charge SKILL #3: Classifying elements - refer to your notes, RB p. 19-25, & the P.T.</p><p>3. Check all the boxes which describe the element. Metal Metalloid Nonmetal Group Group Transitio Halogen Noble Monatomic Diatomic 1 2 n gas metal Sb   Sr    Rn    P   Pt    Cs    S   Fe    Br    Ar    H   Si   B   F    He    Se   Zn    Ra   </p><p>SKILL #4: identifying PROPERTIES OF ELEMENTS – use your notes, RB p. 19-25, Table S & the P.T.</p><p>4. Use Table S to fill in the names and states of each element below. Then, check all the boxes which describe the element. Physical Properties Chemical Properties Conductor Ionization Electro- State at Electrons Name STP Brittl Malleable energy negativity e /ductile Good Poor Low High Low High Los Gain (s, l, or g) e C carbon s      Ag silver s      Mg magnesium s      I iodine s      S sulfur s      Au gold s      Fe iron s      Br bromine l     Ar argon g   H hydrogen g     Hg mercury l     Se selenium s      F fluorine g     He helium g  </p><p>5. Describe one chemical property of Group 1 metals that results from the atoms of each metal having only one valence electron. form 1+ ions; react vigorously with water;easily lose one electron SKILL #5: explaining PROPERTIES OF ELEMENTS – use your notes, RB p. 19-25 & the P.T.</p><p>6. Given: Samples of Na, Ar, As, Rb</p><p> a. Which two of the given elements have the most similar chemical properties? Na and Rb</p><p> b. Explain your answer in terms of atomic structure. They have the same number of valence electrons</p><p>7. Given: Samples of sulfur, oxygen, and phosphorus a. Which two of the given elements have the most similar chemical properties? sulfur and oxygen</p><p> b. Explain your answer in terms of atomic structure. They have the same number of valence electrons</p><p>8. Based on the Periodic Table, explain why Na and K have similar chemical properties. [1] They have the same number of valence electrons form 1+ ions are located in same group</p><p>9. Explain the following in terms of atomic structure: a. Cesium has a larger atomic radius than rubidium. (same group) Cesium has more shells of electrons</p><p> b. Cesium has a lower first ionization energy than rubidium. (same group) Cesium has more electron shells, easier to remove electrons</p><p> c. Bromine has a lower first ionization energy than chlorine. (same group) Br has more electron shells – easier to remove electrons</p><p> d. The atomic radius of copper is 128 picometers while Ag has an atomic radius of 144 picometers. (same group) Ag has one more shell of electrons, so it is larger than Cu</p><p> e. The atomic radius of lithium is 155 pm while neon has an atomic radius of 51 pm. (same period) Neon has more protons in its nucleus which pull the e-‘s in closer.</p><p> f. Lithium has a lower first ionization energy than beryllium. (same period) Lithium has one less proton in its nucleus, so it’s easier to pull an e- away</p><p> g. Chlorine has a greater electronegativity than sulfur. (same period) Chlorine has one more proton in its nucleus, so it’s better at attracting electrons</p><p> h. Potassium has a lower first ionization energy than calcium. (same period) K has one less proton in its nucleus, so it’s easier to pull an e- away</p><p>SKILL #6: identifying TRENDS IN THE PERIDIOC TABLE – refer to your notes, RB p. 26-28, Table S, and the P.T. 10. Base your answers to the following questions on the information below.</p><p> a. Complete the table above. First Ionization Energy of Group 1 Elements b. On the grid below, mark an appropriate Element Atomic First Ionization scale on the axis labeled “First Ionization Energy (kJ/mol).” An appropriate scale is Number Energy (kJ/mol) one that allows a trend to be seen. c. On the grid, plot the data from the table. lithium 3 520 Circle and connect the points. sodium 11 496 potassium 19 419 rubidium 37 403 cesium 55 376 d. State the trend in first ionization energy for the elements in the table as atomic number increases. [1] Ionization energy decreases.</p><p>11. Complete the table below by checking the appropriate boxes. Remember the snow-woman “AMIE” Across a Period  Down a Group  Increases Decreases Increases Decreases Atomic radius   Metallic character   Ionization energy   Electronegativity   # of protons # of electron shells Why? increases increases</p><p>12. Complete the statements below by checking the correct ending. (hint: use Table J for e and f) remains increases decreases the same a. As the elements in a Period are considered from left to right, the  number of valence electrons in each successive element… b. As the elements in Group 17 are considered from top to bottom,  the number of valence electrons in each successive element… c. Going left to right across a Period, the number of electron  shells… d. As the elements in a Group are considered from top to bottom,  the number of electron shells… e. As the elements in Group 1 are considered from top to bottom,  the reactivity of each successive element…. f. As the elements in Group 17 are considered from top to bottom,  the reactivity of each successive element…</p>